Step 1 Identify the concentration-time equation for a first order reaction. Step 2 Calculate the ratio of the concentration after and before reaction. Take the natural log of this ratio. Step 3 Using the natural log of the ratio of concentrations and the time elapsed, calculate the rate constant. The isomerization of methyisocyanide, CH3NC, to acetonitrile, CH3CN, is a first-order reaction. If 2.56 mg of CH3NC is present initially, and 1.89 mg is present after 474 min at 230 what is the value of the rate constant, k? Assume the volume is constant. min-1

Step 1 Identify the concentration-time equation for a first order reaction. Step 2 Calculate the ratio of the concentration after and before reaction. Take the natural log of this ratio. Step 3 Using the natural log of the ratio of concentrations and the time elapsed, calculate the rate constant. The isomerization of methyisocyanide, CH3NC, to acetonitrile, CH3CN, is a first-order reaction. If 2.56 mg of CH3NC is present initially, and 1.89 mg is present after 474 min at 230 what is the value of the rate constant, k? Assume the volume is constant. min-1

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 39QRT

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